Topic 6 - Groups in the Periodic Table

Question 1

What are group 1 elements know as?

Answer 1

The alkali metals

Question 2

What are the properties of group 1 metals?

Answer 2

Low mp/bp

Very soft

Question 3

How reactive are group 1 metals?

Answer 3

Very reactive

Question 4

What determines a metals reactivity?

Answer 4

How readily it loses its outer electron

Question 5

What is the trend of reactivity for group 1?

Answer 5

As you go down, it gets more reactive

Question 6

What happens when alkali metals are put in water?

Answer 6

They react vigorously

Question 7

What is the word equation for the reaction between water and alkali metals?

Answer 7

Alkali Metal + Water -> Metal Hydroxide + Hydrogen

Question 8

How do test for the presence of hydrogen gas?

Answer 8

By a lit splint making a squeaky pop

Question 9

Describe the observations when lithium is put into water?

Answer 9

It will move around the surface, fizzing furiously

Question 10

Describe the observations when sodium is put into water?

Answer 10

It will move around the surface, fizzing furiously whilst also melting due to the heat of the reaction

Question 11

Describe the observations when potassium is put into water?

Answer 11

It will move around the surface, fizzing furiously whilst also igniting the hydrogen gas produced

Question 12

Write a balance symbol equation for the reaction between potassium and water

Answer 12

2K + 2H2O -> 2KOH + H2

Question 13

What are group 7 elements known as?

Answer 13

The halogens

Question 14

What do the halogens exist as?

Answer 14

Diatomic molecules

Question 15

What do you notice as you go down the halogens?

Answer 15

The melting points and boiling points increase

Colour gets darker

Question 16

Describe chlorine

Answer 16

A fairly reactive, poisonous, green gas

Question 17

Describe bromine

Answer 17

A poisonous, red-brown liquid, which gives off an orange vapour at room temperature

Question 18

Describe iodine

Answer 18

A dark grey crystalline solid which gives off a purple vapour when heated

Question 19

How do you test for chlorine?

Answer 19

By holding a piece of damp blue litmus paper which will bleach if chlorine is present, turning it white
It may also turn red for a moment first

Question 20

What is the trend of reactivity for halogens?

Answer 20

Decreases as you go down

Question 21

What is the word equation between metals and halogens?

Answer 21

Metal + Halogen -> Metal Halide

Question 22

What do metals and halogens react to form?

Answer 22

Metal halides

Question 23

What are metal halides?

Answer 23

Salts formed when halogens react with metals

Question 24

What is the word equation between hydrogen and halogens?

Answer 24

Hydrogen + Halogens -> Hydrogen Halide

Question 25

Write a balanced symbol equation for the reaction between bromine and sodium?

Answer 25

Br2 + 2Na -> 2BrNa

Question 26

What is a displacement reaction?

Answer 26

Where a more reactive element displaces a less reactive element from a compound

Question 27

What type of reactions are halogen displacement reactions?

Answer 27

Redox

Question 28

Why are halogen displacement reactions redox?

Answer 28

Because halide ions lose electrons whilst halogens gain elecrons

Question 29

A student adds a few drops of a halogen solution to a potassium iodide solution The solution turned brown Explain what the student should do to help him identify the halogen solution

Answer 29

He should add a few drops of the solution to a bromine salt solution If the solution turns orange, the halogen solution contains chlorine

Question 30

What are group 0 elements?

Answer 30

Inert and colourless gases

Question 31

What are group 0 elements called?

Answer 31

Noble gases

Question 32

What does monatomic mean?

Answer 32

They are gases made up of single atoms

Question 33

Are noble gases diatomic or monatomic?

Answer 33

Monatomic

Question 34

What are the properties of the noble gases?

Answer 34

Monatomic Inert Colourless Non-flammable

Question 35

What are the uses of noble gases?

Answer 35

Stopping burning in filament lamp Welding in metals Airships Balloons

Question 36

Why are noble gases used in filament lamps?

Answer 36

Because they're non-flammable

Question 37

Why does helium float?

Answer 37

Because it's density is lower than air

Question 38

Why is helium used over hydrogen?

Answer 38

Because hydrogen is extremely flammable

Question 39

What is the trend as you go down the noble gases?

Answer 39

Boiling point, melting point and density all increase

Question 40

Use the densities off helium (0.2 kg/m³) and argon (1.8 km/m³) to predict the density of neon

Answer 40

(0.2 + 1.8) / 2 = 2.0 / 2 = 1 | Neon should have a density of about 1.0 kg/m³

Question 41

Give two properties of the group 1 metals?

Answer 41

Low mp/bp | Very soft

Question 42

Explain why group 1 metals are so reactive?

Answer 42

Because all group 1 metals have only 1 outer electron meaning there is only 1 electron that needs to be lost meaning it is very reactive

Question 43

Put all these alkali metals in order of reactivity, staring with the least reactive: Potassium, Caesium, Lithium and Sodium

Answer 43

Lithium, Sodium, Potassium and Caesium

Question 44

How many electrons do halogens have in their outer shell?

Answer 44

7

Question 45

Why can halogen displacement reactions be described as redox reactions?

Answer 45

Because halogens gain electrons whilst the halide ions lose electrons

Question 46

If chlorine water is added to potassium bromide solution, what colour will the solution turn?

Answer 46

Orange solution formed

Question 47

At room temperature, what colour are the Group 0 gases?

Answer 47

Colourless

Question 48

Why are balloons filled with helium able to float in the air?

Answer 48

Because helium has a lower density than air meaning it will float